Name Class Date ELECTRONS AND THE STRUCTURE OF ATOMS

Transcription

1 Name Class Date The Periodic Table ELECTRONS AND THE STRUCTURE OF ATOMS 6.1 Organizing the Elements Essential Understanding Although Dmitri Mendeleev is often credited as the father of the periodic table, the work of many scientists contributed to its present form. Lesson Summary Searching for an Organizing Principle As more and more elements were discovered, scientists needed a way to classify them. Elements were first classified according to their properties. Mendeleev s Periodic Table Mendeleev developed the first periodic table, arranging elements according to a set of repeating, or periodic, properties. Elements were also placed in order, according to increasing atomic mass. Mendeleev used his table to predict the properties of yet undiscovered elements. Today s Periodic Table Today s periodic table is a modification of Mendeleev s periodic table. The modern periodic table arranges elements by increasing atomic number. Periodic law states that when elements are ordered by increasing atomic number, their chemical and physical properties repeat in a pattern. Metals, Nonmetals, and Metalloids Within the periodic table, elements are classified into three large groups based on their properties. Metals are good conductors and many are ductile and malleable. Nonmetals are mostly gases whose properties are opposite to those of metals. Metalloids can behave like metals or nonmetals, depending on the conditions. After reading Lesson 6.1, answer the following questions. Searching for an Organizing Principle 1. How many elements had been identified by the year 1700? 2. What caused the rate of discovery to increase after 1700? 3. What did chemists use to sort elements into groups?

2 Mendeleev s Periodic Table 4. Who was Dmitri Mendeleev? 5. What property did Mendeleev use to organize the elements into a periodic table? 6. Is the following sentence true or false? Mendeleev used his periodic table to predict the properties of undiscovered elements. Today s Periodic Table 7. How are the elements arranged in the modern periodic table? 8. Is the following statement true or false? The periodic law states that when elements are arranged in order of increasing atomic number, there is a periodic repetition of physical and chemical properties. Metals, Nonmetals, and Metalloids 9. Explain the color coding of the squares in the periodic table in Figure Which property below is NOT a general property of metals? a. ductile c. malleable b. poor conductor of heat d. high luster 11. Is the following statement true or false? The variation in properties among metals is greater than the variation in properties among nonmetals. 12. Under some conditions, a metalloid may behave like a. Under other conditions, a metalloid may behave like a. 6.2 Classifying the Elements Essential Understanding A periodic table shows much information about an element in an element s square, and arranges elements by their electron configuration. Lesson Summary Reading the Periodic Table An element s square has the element s symbol and name, atomic number and mass, and electron configuration. The elements are grouped into alkali metals, alkaline earth metals, and halogens. Electron Configurations in Groups The properties of elements are largely determined by the arrangement of electrons, or electron configuration, in each atom. Based on their electron configurations, elements are classified as noble gases, representative elements, transition metals, or inner transition metals.

3 After reading Lesson 6.2, answer the following questions. Reading the Periodic Table 1. Label the sample square from the periodic table below. Use the labels element name, element symbol, atomic number, and average atomic mass. 2. List three things, other than the name, symbol, atomic number, and average atomic mass, you can discover about an element using the periodic table in Figure 6.9. a. b. c. Electron Configurations in Groups 3. Is the following sentence true or false? The subatomic particles that play the key role in determining the properties of an element are electrons. 4. Why are Group A elements called representative elements? 5. Classify each of the following elements as a(n) alkali metal, alkaline earth metal, halogen, or noble gas. a. sodium d. fluorine b. chlorine e. xenon c. calcium f. potassium 6. For elements in each of the following groups, how many electrons are in the highest occupied energy level? a. Group 3A b. Group 1A c. Group 8A 7. Complete the table about classifying elements according to the electron configuration of their highest occupied energy level. Category Description of Electron Configuration Noble gases Representative elements s sublevel and nearby d sublevel contain electrons s sublevel and nearby f sublevel contain electrons 8. Circle the letter of the elements found in the p block. a. Groups 1A and 2A and helium c. transition metals b. Groups 3A, 4A, 5A, 6A, 7A, and 8A except for helium d. inner transition metals

5 13. Use Figure 6.9. Write the electron configurations for the following elements. a. magnesium b. cobalt c. sulfur 6.3 Periodic Trends Essential Understanding An element s properties are related to its position on the periodic table, and these properties follow trends on the table. Lesson Summary Trends in Atomic Size Atomic size is an atom s atomic radius, or one-half the distance between two like atoms when they are joined together. Atomic size generally increases from top to bottom within a group because the number of energy levels increases. Atomic size decreases from left to right across a period because electrons are added to the same energy level and are pulled closer to the nucleus by increasing numbers of protons. Ions Ions form when atoms gain or lose electrons. A positively charged cation forms when an atom loses one or more electrons. A negatively charged anion forms when an atom gains one or more electrons. Trends in Ionization Energy Ionization energy is a measure of how much energy is required to remove an electron from an atom. First ionization energy is the amount of energy required to remove one electron from a neutral atom. Ionization energy tends to decrease from top to bottom within a group and increase from left to right across a period. Trends in Ionic Size Trends in ionic size are based on the fact that metals tend to lose electrons, and nonmetals tend to gain electrons. A cation is smaller than the atom that formed it; an anion is larger than the atom that formed it. Ionic size generally increases from top to bottom within a group and decreases from left to right across a period. Trends in Electronegativity Electronegativity is a measure of an atom s ability to attract an electron when the atom is bonded to another atom. The trends in electronegativity are similar to the trends in ionization energy. Electronegativity tends to decrease from top to bottom within a group and to increase from left to right across a period.

6 0 After reading Lesson 6.3, answer the following questions. Trends in Atomic Size 7. What are the atomic radii for the following molecules? Hydrogen atomic radius = Oxygen atomic radius = Nitrogen atomic radius = Chlorine atomic radius = 8. What is the general trend in atomic size within a group? Across a period? 9. What are the two variables that affect atomic size within a group? a. b. 10. For each pair of elements, circle the element with the larger atom. Ions a. helium and argon b. potassium and argon 11. What is an ion? 12. How are ions formed? 13. An ion with a positive charge is called a(n) ; an ion with a negative charge is called a(n). 14. Complete the table about anions and cations. Anions Cations Charge Metal/Nonmetal Minus sign/plus sign Trends in Ionization Energy 15. is the energy required to overcome the attraction of protons in the nucleus and remove an electron from a gaseous atom. 16. Why does ionization energy tend to decrease from top to bottom within a group? 17. Why does ionization energy tend to increase as you move across a period?

7 18. There is a large increase in ionization energy between the second and the third ionization energies of a metal. What kind of ion is the metal likely to form? Include the charge in your answer. Trends in Ionic Size 19. Metallic elements tend to electrons and form ions. Nonmetallic elements tend to electrons and form ions. 20. Circle the letter of the statement that is true about ion size. a. Cations are always smaller than the neutral atoms from which they form. b. Anions are always smaller than the neutral atoms from which they form. c. Within a period, a cation with a greater charge has a larger ionic radius. d. Within a group, a cation with a higher atomic number has a smaller ionic radius. 21. Which ion has the larger ionic radius: Ca 2+ or Cl? Trends in Electronegativity 22. Use Table 6.2. What trend do you see in the relative electronegativity values of elements within a group? Within a period? 23. Circle the letter of each statement that is true about electronegativity values. a. The electronegativity values of the transition elements are all zero. b. The element with the highest electronegativity value is sodium. c. Nonmetals have higher electronegativity values than metals. d. Electronegativity values can help predict the types of bonds atoms form. 24. Use Figure Circle the letter of each property for which aluminum has a higher value than silicon. a. first ionization energy c. electronegativity b. atomic radius d. ionic radius

8 Name Class Date 6 Self-Check Activity For Questions 1 11, complete each statement by writing the correct word or words. If you need help, you can go online. 6.1 Organizing the Elements 1. Early scientists first sorted elements into groups according to their. 2. In Mendeleev s periodic table, elements were arranged by increasing. 3. Currently, elements are arranged on the periodic table according to increasing. 4. Each element is either a metal, a(n), or a metalloid. 6.2 Classifying the Elements 5. The periodic table contains much information about the elements, including their, names, and information about the structure of their atoms. 6. Elements can be sorted into groups with similar properties based on their. 6.3 Periodic Trends 7. Atomic size increases from top to bottom within a(n) and from left to right across a(n) of the periodic table. 8. with a positive or negative charge forms when electrons are transferred from one atom to another. 9. The first ionization energy of atoms tends to from top to bottom within a group and from left to right across a period. 10. When an atom loses one or more electrons to form an ion, the ion is than the original atom; when an atom gains one or more electrons to form an ion, the ion is than the original atom. 11. Trends in electronegativity follow the same pattern as trends in. If You Have Trouble With Question See Page

9 Name Class Date Review Vocabulary Match each of the following with its location on the periodic table, using letters a i. Use each choice only once. 1. alkali metals 2. alkaline earth metals 3. halogens 4. inner transition metals 6. metals 7. noble gases 8. nonmetals 9. transition metals 5. metalloids Use the letters j m to show periodic trends in the following properties. The arrows point in the direction the properties increase. Two letters should be in each blank. 10. atomic radius 11. electronegativity 13. size of anion 14. size of cation 12. ionization energy

6 THE PERIODIC TABLE SECTION 6.1 ORGANIZING THE ELEMENTS (pages 155 160) This section describes the development of the periodic table and explains the periodic law. It also describes the classification

Chapter 6 The Periodic Table Organizing the Periodic Table In a grocery store, the products are grouped according to similar characteristics. With a logical classification system, finding and comparing

The Periodic Table Organizing the Elements A few elements, such as gold and copper, have been known for thousands of years - since ancient times Yet, only about 13 had been identified by the year 1700.

Unit 5 Elements and their Properties 1. In 1871, Russian chemist Mendeleev created the forerunner of the modern periodic table. 2. The elements in Mendeleev's table were arranged in order of increasing

Review- The Periodic Table Name Date Block Matching: Match the description in with the correct term in. Write the letter in the blank provided. Each term matches with only one description, so be sure to

Chapter 5: The Periodic Law Section 5.1: The History of the Periodic Table Dmitri Mendeleev (1869) first person to organize the elements in a chart Organized about 70 elements by increasing atomic mass

Trends of the Periodic Table Diary Trends are patterns of behaviors that atoms on the periodic table of elements follow. Trends hold true most of the time, but there are exceptions, or blips, where the

ATOMIC STRUCTURE AND THE PERIODIC TABLE CHAPTER 4 WORKSHEET PART A Given the following isotopes, determine the atomic number, the mass number, the number of protons, electrons and neutrons. Isotope Symbol

Name: Class: Date:, ID: A The Periodic Table Multiple Choice Identify the choice that best completes the statement or answers the question: 1. What are the elements with atomic numbers from 58 to 71 called?

Chapter 5 TEST: The Periodic Table name HPS # date: Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The order of elements in the periodic table is based

Periodic Table Extra Practice 1. Which of the following elements in Period 3 has the greatest metallic character? 1) Ar 3) Mg 2) Si 4) S 2. Which sequence of atomic numbers represents elements which have

Material: laboratory display of the elements and a wall periodic table is required. Objective: To learn the use of periodic table for writing electron configuration of elements. INTRODUCTION Basic building

Unit 3 Review Chapters 4 (Atomic Structure) & 6 (Periodic Table) Part 1: Answer the following questions. 1. a. Which scientist created the first modern atomic theory? John Dalton b. What was his theory?

Chemistry: The Periodic Table and Periodicity Name: Hour: Date: Directions: Answer each of the following questions. You need not use complete sentences. 1. Who first published the classification of the

Chemistry: The Periodic Table and Periodicity Name: per: Date:. 1. By what property did Mendeleev arrange the elements? 2. By what property did Moseley suggest that the periodic table be arranged? 3. What

Unit 6 Particles with Internal Structure 3-1 The Elements Remember, elements are combined to form molecules the way letters are combined to form words. Presently there are about 115 known elements. Only

Unit 3.2: The Periodic Table and Periodic Trends Notes The Organization of the Periodic Table Dmitri Mendeleev was the first to organize the elements by their periodic properties. In 1871 he arranged the

The Periodic Table Horizontal Rows are called Periods. Elements in the same period have the same number of energy levels for ground state electron configurations. Vertical Rows are called Families or Groups.

Periodic Table Instructional Background Patterns in Element Properties (History): Elements vary widely in their properties, but in an orderly way. In 1869, the Russian chemist Dmitri Mendeleev produced

The following are topics and sample questions for the first exam. Topics 1. Mendeleev and the first periodic Table 2. Information in the Periodic Table a. Groups (families) i. Alkali (group 1) ii. Alkaline

1. Which statement best describes Group 2 elements as they are considered in order from top to bottom of the Periodic Table? (A) The number of principal energy levels increases, and the number of valence

Periodic Table and Trends Test Review KEY Describe the common characteristics and uses of the following families: 1. Alkali metals (# of valence electrons = 1) Most reactive metals that do not occur freely

Date: Science 10 4.1 Atomic Theory & Bonding What is an Atom? smallest particle of an element that still has the properties of that element An atom = proton(s) + electron(s) + neutron(s) (PEN) Fun Fact:

Lesson Outline for Teaching Lesson 1: Using the Periodic Table A. What is the periodic table? 1. The periodic table is a chart of the elements arranged into rows and columns according to their chemical

Matter and the Periodic Table Purpose The purpose of this station is to reinforce students understanding of the organization and predictive power of the Periodic Table of the Elements and students ability

Periodic Table Questions 1. The elements characterized as nonmetals are located in the periodic table at the (1) far left; (2) bottom; (3) center; (4) top right. 2. An element that is a liquid at STP is

Name Chemistry-PAP Period I. History Notes: Periodic Table and Periodic Trends Dmitri Mendeleev (1836-1907) Russian professor Gathered a wealth of data on all chemical elements known at the time noticed

PERIODIC TABLE NOTES (from chapters 5 and 6) I. History of the Periodic Table As the number of elements began to grow, chemists needed a way to all of these elements. [In the 1700 s there were known elements.

Periodic Table Science 7 2015 ??? From an elements location in the periodic table, you can predict properties From an elements location in the periodic table, you can predict ??? Most metals are this state

Students will be able to read the periodic table, define atom, molecule, and element, and construct a model of an atom and molecule. Vocabulary Atom- smallest part of an element that retains the properties

Valence Electrons Everything that is underlined should get filled in on your notes! Valence Electrons Valence electrons the electrons that are in the highest (outermost) energy level that level is also

Isotopes Isotopes are atoms of the same element that have different masses due to different numbers of neutrons. See the example below for two isotopes of oxygen. One has 8 neutrons while the other has

Trends of the Periodic Table Basics Trends are patterns of behaviors that atoms on the periodic table of elements follow. Trends hold true most of the time, but there are exceptions, or blips, where the

PERIODIC TABLE OF ELEMENTS, a Russian scientist is credited with creating the periodic table. Periods tell us how many are in the atoms of each element. Groups help us to know how many electrons are in

The Periodic Table of The Elements Elements are like a collection As more and more elements were discovered it became more important to organize and classify them Between the late 1700 s and mid 1800 s

Name: Date: 1. Which of the following best describes an atom? A. protons and electrons grouped together in a random pattern B. protons and electrons grouped together in an alternating pattern C. a core

1. Atoms of elements that are in the same group have the same number of 5. Mendeleev left gaps in his periodic table because A. Protons B. Valence Electrons A. the table was too full B. no known elements

Unit 2 Periodic Behavior and Ionic Bonding 6.1 Organizing the Elements I. The Periodic Law A. The physical and chemical properties of the elements are periodic functions of their atomic numbers B. Elements

Periodicity and the Periodic Table the result Dmitri Mendeleev arranged elements in order of their atomic numbers, such that elements with similar properties fell into the same column or group. The Periodic

Chapter 17 Assessment Please write you answers on a separate piece of paper. Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Mendeleev created

1. Which characteristics describe most nonmetals in the solid phase? (1) They are malleable and have metallic luster. (2) They are malleable and lack metallic luster. (3) They are brittle and have metallic

The Periodic Table Bromfield Honors Chemistry Write your answers in your notebook What is a trend? What are some patterns or trends you have observed? Periodic Law Historical development Chemical Periodicity

1 The Periodic Table Scientists had identified certain substances as elements and so there were many attempts to arrange the known elements so that there were some correlations between their known properties.

Chemistry Unit 5- Periodic Table and Periodic Law Name: History of the Periodic Table I. Mendeleev and Chemical Periodicity A. Wanted to organize elements according to their B. When elements were arranged

EXPERIMENT 4 The Periodic Table - Atoms and Elements INTRODUCTION Primary substances, called elements, build all the materials around you. There are more than 109 different elements known today. The elements

HIGH SCHOOL SCIENCE Physical Science 10: Periodic Table WILLMAR PUBLIC SCHOOL 2013-2014 EDITION CHAPTER 10 Periodic Table In this chapter you will: 1. Describe how Mendeleev arranged the elements in his

Name Regents Chemistry 2014-15 Unit 2 - The Periodic Table This unit will be both quick and easy, serving as a bridge between two very challenging units. Objectives: At the end of this unit, students will:

Do Now: What is the Periodic Table? The Periodic Table History Dmitri Mendeleev Mendeleev s Proposal Arranged the elements into rows in order of increasing mass and placed elements with similar properties

3.93 Give the period and group number for each of the following elements: a. bromine b. argon c. potassium d. radium 3.94 Give the period and group number for each of the following elements: a. radon b.

Name: Period: Date: Unit 3 Review: things you will need to know 1. Atomic Theories: Know all the scientists in order. What did they discover? What experiment did they use? 2. Development of the periodic

CHAPTER OUTLINE Section 1 Organizing the Elements Key Idea questions > How did Mendeleev arrange the elements in his periodic table? > How are elements arranged in the modern periodic table? Recognizing

1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and

CHEM100 Week 4 Notes Page 1 of 6 Scientists create models to understand how things work, including atoms. Dalton created a theory for the atom with these 5 postulates 1. Elements consist of one or more

Chemistry 25 Chapter 4 Atoms and Elements Experiencing Atoms What is ATOM? Atoms are incredibly small, yet they compose everything. Atoms are the pieces of elements. Properties of the atoms determine the

1 Pre-Test : Atomic Structure and the Periodic Table Directions: Circle the letter to indicate whether the following statements are either true ( T ) or false ( F ). 1. Atomic structure refers to the building

UNIT-3 Classification of elements and periodicity in properties One mark questions:. For the triad of elements A, B and C if the atomic weights of A and C are 7 and 39. Predict the atomic weight of B..

The Periodic Table Section 1 How Are Elements Organized? Section 2 Tour of the Periodic Table Section 3 Trends in the Periodic Table Section 4 Where Did the Elements Come From? Section 1 How Are Elements

Chapter 7 Periodic Properties of the Elements 1. Elements in the modern version of the periodic table are arranged in order of increasing. (a). oxidation number (b). atomic mass (c). average atomic mass

Name: Date: 1. In the modern Periodic Table, the elements are arranged in order of increasing A. atomic number B. mass number C. oxidation number D. valence number 6. As the elements in Group IA are considered

Question (1) Chapter Two Periodic Table Choose the correct answer for each statement of the following:- 1- The elements of same vertical group are identical in the number of----------- a valence electrons

Question 1: Did Dobereiner s triads also exist in the columns of Newlands Octaves? Compare and find out. Only one triad of Dobereiner s triads exists in the columns of Newlands octaves. The triad formed